. The decomposition of N₂O5 in carbon tetrachloride has been studied:2 N₂O5 (g) → 2 N₂O4 (g) + O₂(g)The concentration of N₂O5 is monitored for 1200 seconds andmeasured every 400 seconds. The data are tabulated below:[N₂O5](M)0.01.40400.01.10800.00.871200.00.68(a) Fill the blanks in the table. Note that the last column is theaverage rate of reaction.(b) Briefly explain why the rates are decreasing.time(s)At(s)Rate =-A[N₂O5]/At(M/s)A[N₂O5](M)

∆t(s) = Final time(s) - Initial time(s) ∆[N2O5] = Final [N2O5] - Initial [N2O5]

The decomposition of N₂O5 in carbon tetrachloride has been studied: 2 N₂Os (g) ->>> 2 N₂O4 (g) + O₂(g) The concentration of N₂O5 is monitored for 1200 seconds and measured every 400 seconds. The data are tabulated below: time(s) [N₂O5] (M) 1.40 At(s) A[N₂O5](M) - Rate =L A[N₂O5]/At(M/s) - 0.0 400.0 1.10 800.0 0.87 1200.0 0.68 (a) Fill the blanks in the table. Note that the last column is the average rate of reaction. (b) Briefly explain why the rates are decreasing. --

The decomposition of N₂O5 in carbon tetrachloride has been studied: 2 N₂Os (g) ->>> 2 N₂O4 (g) + O₂(g) The concentration of N₂O5 is monitored for 1200 seconds and measured every 400 seconds. The data are tabulated below: time(s) [N₂O5] (M) 1.40 At(s) A[N₂O5](M) - Rate =L A[N₂O5]/At(M/s) - 0.0 400.0 1.10 800.0 0.87 1200.0 0.68 (a) Fill the blanks in the table. Note that the last column is the average rate of reaction. (b) Briefly explain why the rates are decreasing. --

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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